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2.4 Concentrated nitric acid used in laboratory work is 68 % n

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$2.4$ Concentrated nitric acid used in laboratory work is $68%$ nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is $1.504 g mL^{- 1}$ ?

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Updated on: Oct 21, 2023

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Evelyn Discussed

2.4

Concentrated nitric acid used in laboratory work is

68%

nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is

1.504 g mL^{- 1}

13 mins ago

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Question Text	$2.4$ Concentrated nitric acid used in laboratory work is $68%$ nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is $1.504 g mL^{- 1}$ ?
Updated On	Oct 21, 2023
Topic	Mole Concept & Redox
Subject	Chemistry
Class	Class 12
Answer Type	Video solution: 34
Upvotes	3133
Avg. Video Duration	6 min

$2.4$ Concentrated nitric acid used in laboratory work is $68%$ nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is $1.504 g mL^{- 1}$ ?

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2.4 Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is 1.504 g mL−1 ?

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$2.4$ Concentrated nitric acid used in laboratory work is $68%$ nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is $1.504 g mL^{- 1}$ ?